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Chapter 5: Problem 20

Based on its position in the periodic table, what is the valence shell and what is the core charge for C? Explain your reasoning.

Short Answer

Expert verified
The valence shell for Carbon is the second energy level, and the core charge is +4.

Step by step solution

01

- Locate the position of Carbon

In the Periodic Table, find Carbon (C). Carbon is in the second row (period) and fourth column (group) in the Periodic Table. This is necessary to determine the valence shell and core charge of the atom.
02

- Identify the Valence Shell

The valence shell is the outermost shell of an atom in its uncombined state, which contributes to or influences its chemical properties. It can be determined from the period number of the element. For Carbon, it is in the second period, so the valence shell is the second energy level.
03

- Determine the Core Charge

The core charge of an atom is the effective nuclear charge experienced by the outermost electrons. It can be calculated as the atomic number minus the number of total inner shell electrons. For Carbon, which is atomic number 6, there are two inner-shell electrons (from the 1st energy level), so the core charge is \(6 - 2 = 4\).

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Most popular questions from this chapter

How many electrons are in the valence shell of a) H? b) Li? C) He?

Locate \(\mathrm{F}\) and \(\mathrm{Cl}\) on the periodic table. a) Describe any relationship between the core charge of these atoms, the number of valence electrons, and their position in the periodic table. b) Describe any relationship between the valence shell of these atoms and their position in the periodic table. c) Within our model and referring to the Coulombic Potential Energy expression, explain why the \(\mathrm{IE}_{1}\) of \(\mathrm{Cl}\) is less than that of \(\mathrm{F}\).

Within our model and referring to the Coulombic Potential Energy expression, explain why the IE increases from left to right across a row of the periodic table.

Assuming that the valence shells of \(\mathrm{Li}\) and \(\mathrm{Be}\) are at approximately the same distance from their nuclei, explain how the core charges of \(\mathrm{Li}\) and \(\mathrm{Be}\) are consistent with the \(\mathrm{IE}_{1}\) values for \(\mathrm{Li}(0.52 \mathrm{MJ} / \mathrm{mole})\) and Be \((0.90 \mathrm{MJ} / \mathrm{mole})\).

What is the core charge of Li?
See all solutions

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